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A sample that weighs 107.75 g is a mixture of 30% helium atoms and 70% krypton atoms. How many particles are present in the sample?
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Ch.3 - Mass Relationships in Chemical Reactions
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
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McMurry 8th EditionCh.3 - Mass Relationships in Chemical ReactionsProblema 57c
McMurry 8th EditionCh.3 - Mass Relationships in Chemical ReactionsProblema 57cCapitolo 3, Problema 57c
What is the mass in grams of each of the following samples? (c) 0.0015 mol of diazepam (Valium), C16H13ClN2O
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Determine the molar mass of diazepam (C_{16}H_{13}ClN_{2}O) by adding the atomic masses of all the atoms in the molecular formula.
Calculate the molar mass: (16 \(\times\) \(\text{atomic mass of C}\)) + (13 \(\times\) \(\text{atomic mass of H}\)) + (1 \(\times\) \(\text{atomic mass of Cl}\)) + (2 \(\times\) \(\text{atomic mass of N}\)) + (1 \(\times\) \(\text{atomic mass of O}\)).
Use the formula: \(\text{mass}\) = \(\text{moles}\) \(\times\) \(\text{molar mass}\) to find the mass in grams.
Substitute the given number of moles (0.0015 mol) and the calculated molar mass into the formula.
Perform the multiplication to find the mass in grams of the diazepam sample.
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Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in a molecule. For example, the molar mass of diazepam (C16H13ClN2O) can be determined by adding the atomic masses of carbon, hydrogen, chlorine, nitrogen, and oxygen in the molecular formula.
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02:11
Molar Mass Concept
Mole Concept
The mole is a fundamental unit in chemistry that quantifies the amount of substance. One mole contains Avogadro's number of entities, approximately 6.022 x 10^23. This concept allows chemists to convert between the number of particles (atoms, molecules) and the mass of a substance, facilitating calculations in stoichiometry and chemical reactions.
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01:25Mole Concept
Conversion between Moles and Grams
To convert moles of a substance to grams, the formula used is: mass (g) = number of moles × molar mass (g/mol). This relationship is essential for determining the mass of a sample when the number of moles is known, as in the case of calculating the mass of 0.0015 mol of diazepam using its molar mass.
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02:28Mass and Moles Conversion
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